1 / 17

THE TRANSITION ELEMENTS

THE TRANSITION ELEMENTS. THE TRANSITION ELEMENTS Position & properties in the P/table: Between highly electropositive and electronegative elements. Defn: Elements having partially filled d or f shells in any common oxdn state (i.e. as neutral atoms or in any oxdn state). E.g.

mariasherman
Download Presentation

THE TRANSITION ELEMENTS

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. THE TRANSITION ELEMENTS

  2. THE TRANSITION ELEMENTS • Position & properties in the P/table: Between highly electropositive and electronegative elements. • Defn: Elements having partially filled d or f shells in any common oxdn state (i.e. as neutral atoms or in any oxdn state). E.g. 1. CuII = [Ar]3d9 Vs Cu0 = [Ar]3d104s1 2. AgII = [Kr]4d9 Vs Ag0 = [Kr] 4d105s1 3. AuIII = [Xe]4f14 5d8 Vs Au0 = [Xe]4f14 5d106s1 4. ZnII = [Ar]3d10Vs Zn0 = [Ar]3d104s2 5. CdII = [Kr]4d10Vs Cd0 = [Kr]4d105s2 6. HgII = [Xe]4f145d10Vs Hg0 = [Xe]4f145d10 7. ScIII = [Ar] Vs Sc0 = [Ar]4s23d1

  3. Three groups of Transition elements are recognized: (1) The main Transition elements or d-block elements. (2) The Lanthanide elements (3) The Actinide elements. • The main Transition d-block elements. (a) The First Transition series Sc= [Ar]4s23d1 = Lightest member Sc Ti V Cr Mn Fe Co Ni and Cu Cu = [Ar]3d104s1 • Have partially filled 3d shells either in the ground state of the free atom [All EXCEPT Cu] or in one or more of their chemically important ions [ALL EXCEPT Sc]. Note: from Zn = 3d104s2 until next 9 elements = NON-TRANSITION

  4. The second Transition series From Yttrium = [Kr] 5s24d1 Y Zr Nb Mo Tc Ru Rh Pd Ag & [Cd non-trans] All have partially filled 4d shells either in the free element [ALL EXCEPT Ag] or in one or more of the chemically important ions [ALL EXCEPT Y]. • The Third Transition series. The Third Transition series starts with Hf = [Xe] 6s25d2. [Xe]4f146s15d10 Hf Ta W Re Os Ir Pt Au & [Hg non-trans]  All have partially filled 5d shells in one or more of their chemically important oxidation states as well as in the neutral atom [EXCEPT Au].

  5. The Lanthanide elements  Starts with Lanthanum = [Xe] 5d16s2. • Next 14 elements electrons enter the 4f shell until Lu (Lutetium). Ce = [Xe]4f15d16s2 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu = [Xe]4f145d16s2. • 5d1electron in Ce, Gd & Lu, in all others this electron is shifted to the 4f orbital. The elements La – Lu have very similar chemical and physical properties. • Those of Lanthanum are prototypal and hence the elements are called the LANTHANIDES.

  6. The Actinide elements. Starts with Ac = [Rn]6d17s2 = Actinium • The difference in energy btn 5f & 6d orbitals in the beginning of the series is less than that btn the 4f & 5d orbitals for the lanthanides. • For Elements immediately following Ac and their ions there may be electrons in 5f or 6d or both (i.e. 5f & 6d are involved in accommodating successive electrons). • After FOUR or FIVE more electrons have been added to the Ac configuration, the 5f orbitals become more stable (Plutonium is reached). Ac Th Pa U Np Pu Am cm Bk Cf Es Fm Md No Lr.

  7. Differences between the Three classes of Transition elements. • D-block elements Partially filled 3d, 4d or 5d orbitals.  Electrons occupying them are strongly influenced by the surroundings and vice versa. ORBITALS PROJECT TO PERIPHERY OF ATOMS. • The Lanthanides Partially filled 4f orbitals.  Electrons occupying them are largely screened from the surroundings by the overlying shells [5s, 5p] of electrons.  4f orbitals deeply buried in atoms/ions

  8. RESULT: • Chemistry of Lanthanides  Homologous • Chemistry of d-block elements. Errate and Irregular variations in chemical properties through a series of d-block elements. • The Actinide elements. - Behaviour lies between d-block and the Lanthanides. - 5f orbitals  not so exposed as the d orbitals and not so well shielded as 4f orbitals.

  9. Factors affecting the stability of Electronic configurations: • Effective nuclear charge. • In hydrogen all the subshells of each principal shell are equi-energetic (one electron atom). • Multi-electron atoms  Energies of subshell depend on the populations of all the other levels. The s, p, d, f etc subshells split apart and drop to lower energies. REASON: Steady increase in the Effective Nuclear charge. • Each electron is IMPERFECTLY SHIELDED from the nuclear charge by other electrons.

  10. Direct interactions between electrons (Interelectronic forces). e.g. Special stability of half filled shells. i.e. Cr = [Ar] 4s13d5 1st Transition series. Cu = [Ar] 4s13d10 Gd = [Xe] 4f76s25d1 Lanthanide. Thus inter electronic forces and variations in total nuclear charge play a large part in determining the configurations of ions. e.g. 4s Occupied before 3d but are not always the more stable. • Elements of the First Transition series ionize by the loss of the 4s first instead of the 3d. e.g. Cu = [Ar] 4s13d10 & Cu2+ = [Ar] 3d9. • Stability of an electronic configuration is determined by • Nuclear-electronic attraction • Shielding of one electron by others • Interelectronic repulsions • Exchange energy of half filled shells.

  11. General Properties: • They are all metals • They are almost all hard, strong, high-melting, high-boiling metals that conduct heat and electricity well. • They form alloys with one another and with other metallic elements. • Many of them are sufficiently electropositive to dissolve in mineral acids although a few are “noble” • With very few exceptions, they exhibit variable valence. • Their ions and compounds are coloured in one if not all oxidation states (with very few exceptions). • Due to partially filled shells, they form some paramagnetic compounds. • They form complex compounds (coordination compounds/ions). Periodic trends in properties: • Atomic radii, Atomic volume and density. • Ionisation energy and Electronegativity. • Melting and Boiling points.

  12. 3.Elements in higher oxidation states are very polarizing and can exist only in an environment of highly electronegative atoms (oxyanions or binary compds of oxygen and fluorine). e.g. +6 for Cr is found in CrO42- +6 for Mo is found in MoO42- +6 for W is found in WO42-

  13. OXIDATION STATES (i) The II state: • All the elements TiCu form well defined binary compds in the DIVALENT STATE. These are essentially ionic e.g. MX2. • Aqua ions are well defined: [M(H2O)6]2+ except Ti. (ii) The III state: • All the elements form at least some compds in this state (Highest for Cu). e.g. Ti2O3, CrF3. • Fluorides and oxides are generally ionic. Chlorides may have considerable covalent character e.g.. FeCl3.

  14. THE LANTHANIDES La Ce Pr Nd Pm SmEuGd Tb Dy Ho Er Tm Yb Lu. They are also known as Lanthanoids or Lanthanon elements. Commercially important minerals. • Monazine=mixed La • Bastnaesite= La LARGEST NATURAL OCCURING GROUPS The Lanthanides are strictly the 14 elements that follow Lanthanum in the Periodic Table, in which fourteen 4f electrons are successively added to the Lanthanum configuration. • Prime Oxidation state = M3+ • La = [Xe]5d16s2 Lu = [Xe]4f145d16s2 The Lanthanide contraction This is the significant and steady decrease in the size of atoms and ions of the Lanthanides with increasing atomic number (z).  Due to imperfect shielding of one electron by another in the same SUBSHELL.

  15. Note: The largest decrease occurs with the first f electrons added and also after f7. • Elements  highly electropositive. Prime Ox. State = +3 • sum of first THREE ionization energies is relatively Low. • They form [M(H2O)n]3+ • Ce can form Ce4+ • Sm, Eu, Yb and Tm can form M2+. Some properties of the Lanthanides. • The metals are very reactive. • Heating with Halogens give LnX3. • They all react directly with water, slowly in the cold, rapidly on heating liberating H2 • React exothermically with hydrogen though heating to 300-400oC is often required to initiate the reaction • Eu and Yb dissolve in liquid ammonia at –78oC giving blue solutions. These solutions are those expected for M2+ ions and solvated electrons.

  16. THE TRIVALENT STATE • This is the characteristic oxidation state for all the lanthanides. • They form (i) Oxides and hydroxides resembling the Ca Ba group ie M2O3 and M(OH)3. - Basicity decrease with increasing atomic number. • MX3 ionic halides • M2S3 and MX (X = N, P, As, Sb or Bi).

  17. THE TETRAVALENT STATE (1) Ce(IV) is the only +4 Lanthanide ion that exist in aqueous solution as well as in the solid state. • Compounds: CeO2 (Ceric Oxide), CeO2.nH3O, (Hydrous Ceric Oxide), CeF4. • Pr (Praseodymium), Tb (Terbium) and Eu (Europium) solid compounds of oxidation state IV are known. eg. NaPrF5, PrF4, TbO2, TbF4 Cs3 NdF7. THE DIVALENT STATE Aqueous solutions and solid compounds of Sm2+, Eu2+ and Yb2+ are known. Solid compounds of M3+ OF Nd, Sm, Dy, Yb and Tm are known but are unstablein water. Eg. NdBr2, SmBr2. Oxides NdO and SmO ( both golden yellow) and EuO (dark red0 YbO SOME USES OF THE LANTHANIDES/LANTHANOIDS • Additives in special purposes steels. Eg making pipes • Catalysis(mixed metal oxides are used) • The phosphorus

More Related